Part B How many moles of nitrogen, N , are in 72.0 g of nitrous oxide, \( \mathrm{N}_{2} \mathrm{O} \) ? Express your answer with the appropriate units. Viow Available Hint(s) Value

1. First, calculate the molar mass of nitrous oxide, \( \mathrm{N_2O} \). The atomic mass of nitrogen is approximately \( 14.0 \, \mathrm{g/mol} \) and that of oxygen is approximately \( 16.0 \, \mathrm{g/mol} \). Thus, the molar mass is \[ M = 2(14.0) + 16.0 = 28.0 + 16.0 = 44.0 \, \mathrm{g/mol}. \] 2. Determine the number of moles of \( \mathrm{N_2O} \) in \( 72.0 \, \mathrm{g} \) using: \[ n_{\mathrm{N_2O}} = \frac{72.0 \, \mathrm{g}}{44.0 \, \mathrm{g/mol}} \approx 1.636 \, \mathrm{mol}. \] 3. Each molecule of \( \mathrm{N_2O} \) contains 2 atoms of nitrogen. Therefore, the number of moles of nitrogen atoms is: \[ n_{\mathrm{N}} = 2 \times n_{\mathrm{N_2O}} = 2 \times 1.636 \approx 3.27 \, \mathrm{mol}. \] The final answer is \( 3.27 \, \mathrm{mol\, N} \).